Answer : The value of [tex]K_b[/tex] is, [tex]7.7\times 10^{-8}[/tex]
Explanation :
As we are given : [tex]K_a=1.3\times 10^{-7}[/tex]
As we know that,
[tex]K_a\times K_b=K_w[/tex]
where,
[tex]K_a[/tex] = dissociation constant of an acid = [tex]1.3\times 10^{-7}[/tex]
[tex]K_b[/tex] = dissociation constant of a base = ?
[tex]K_w[/tex] = dissociation constant of water = [tex]1\times 10^{-14}[/tex]
Now put all the given values in the above expression, we get the dissociation constant of a base.
[tex]1.3\times 10^{-7}\times K_b=1\times 10^{-14}[/tex]
[tex]K_b=7.7\times 10^{-8}[/tex]
Therefore, the value of [tex]K_b[/tex] is, [tex]7.7\times 10^{-8}[/tex]
